D'Agostin: Unit #6 Notes - Bonding & Lewis Dot Structures

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Bonding & Lewis Dot StructuresUnit #4 NotesSingle Covalent BondA bond in which 2 atoms share a pair of valence electrons.Double Covalent BondTriple Covalent BondA bond in which 2 atoms share 3 pair of valence electrons.A bond in which 2 atoms share 2 pair of valence electrons.Lewis Dot StructureDescribe the number of bonds found in a molecule and the arrange of unshared pairs (lone pairs) of electrons.1. Determine the total # of valence electrons.2. Write the symbols of the atoms in the molecule. The central atom must be able to form more than 1 bond.3. Draw 2 dots to represent a chemical bond.4. No atom should have more that 8 valence electrons.Octet RuleRemember, covalent bonds form so that each atom that is part of a molecule has a complete set of 8 valence electrons.Bond PolarityDescribes the degree to which a pair of electrons is shared between the 2 atoms that are part of a chemical bondNonpolar Covalent BondPolar Covalent BondA covalent bond that forms if the 2 atoms do NOT share a pair of valence electrons equally. This type of bond results in an unequal distribution of charge because 1 of the atoms has a greater share of the electron pair.Ionic BondThe bond formed between large numbers of cations (+ ions) and anions (- ions)

Remember, opposite charges attract!A covalent chemical bond formed if 2 atoms share a pair of valence electrons equally. This type of bond results in a balanced distributionof charge.ElectronegativityA measure of an atoms ability to attract electronsLone PairorUnshared PairAn atom has a greater share of the electron pair if it has a higher electronegativity